Physical Chemisty

Maria Grzeszczuk, prof. dr hab.
Number of hours: 
2h X 15 weeks = 30 hours (1 semester)
Number of hours: 
3h X 15 weeks = 45 hours (1 semester)
Number of hours: 
3h X 15 weeks = 45 hours (1 semester)

The purpose of the lectures, seminars and laboratories is to gain by students the basic theoretical and experimental information about physical chemistry. The lessons are divided into four parts: thermodynamics, chemical and phase equilibria, electrochemistry and chemical kinetics.

Acquired Knowledge
- knows the basics of physicochemical descriptions and analyzes physical phenomena and chemical processes, using adequate mathematical apparatus
- is in the possession of basic aspects of the actions of scientific equipment
Acquired Skills
- Student is able to use numerical methods to solve physicochemical problems and for experimental data analysis,


Lecture: written exam (obligatory) + oral exam (additional/optional)
Seminar: solving of selected problems and calculus from an early known list provided each week, passing of two written tests per semester
Laboratory: oral colloquia (obligatory) and written reports (obligatory) on the selected laboratory exercises


Completed mathematics course


Chemical kinetics, electrochemistry


Chemical kinetics: fundamental terminology and definitions, the rate law, kinetic parameters, simple and complex reactions, fundamental mechanistic-kinetic schemes. Temperature dependence of the reaction rate, Arrhenius parameters. Effect of pressure on the reaction rate. Molecular reaction dynamics. Elementary reactions and molecular mechanisms. The enthalpy and entropy of activation. Kinetics of selected complex reactions: square scheme reactions, chain reactions, enzymatic reactions, reactions with adsorbed reactants. Adsorption - thermodynamic-kinetic aspects, isotherms (Langmuir, BET)

Electrochemistry: electrochemical systems as dynamic multi-component, multi-phase systems and interfacial processes. Fundamentals of electrochemical kinetics. Electrode reactions and processes, electrode potentials and currents, membrane potentials. Standard and equilibrium potentials. The Nernst equation. The electromotive force of galvanic cell and selected practical cells and thermodynamics. The voltage of electrolytic cells. Electric conductivity of electrolytes. Debye-Huckel-Onsager theory. Molecular interactions and transport properties of molecules in liquids. Transport parameters: diffusion coefficient, ion mobility, viscosity.


Kinetics - the rate of basic reactions

Determination of order of reaction, half-time and rate constant

The rate of reactions areaching equilibrium, parallel reactions, consecutive reactions

Steady-state approximation, mechanism of reactions

Enzymatic reactions, Michaelis-Menten mechanism


Types of galvanic cells, Nernst equation

Thermodynamics of galvanic cells

Activity coefficients, Debye-Hückel equation

Conductivity of electrolytes, Kohlrausch equation


Dipolar moments

Refractometric titration

Parameters of the absorption band

Electromotive force (EMF) of electrochemical cells

Thermodynamics of electromotive cells

Conductivity of electrolytes

Viscosity of a liquid

Transport numbers of ions

Acidolysis of ester

Kinetics of the saccharose inversion

Kinetic salt effect of the ionic reaction

The Surface Tension of a Liquid

Temperature sensors